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calculate the pH of the solution formed by mixing 10.0ml of 0.15M HBr with 20.0ml of 0.25M HCl
concentration of [H+] (from HBr and HCl) n(H+) = 0.15*10/1000 + 0.25*20/1000=0,0065 mol in 30 ml x mol in 1000 ml x=0.217 [H+]=0.217M
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Calculate the Qsp for the mixing of 30.0mL of 3.7 × 10^-3 M Sr(NO3)2 and 25.0mL of 0.02 M Na2SO4
Qsp of SrSO4 = Concentration of Sr2+ × Concentration of SO42- .= ( 30 × 3.7 × 10-6 ) / 55 × 10-3 × ( 25 × 0.02 ×...
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35.6 ± 0.4 mL of 0.600 ± 0.02 M HCl was required to neutralize 35 ± 0.3 mL of a solution of NaOH. Calculate the error in the concentration of NaOH in M from the combined errors in the data.
Concentration of NaOH = Volume of HCl × Concentration of HCl/Volume of NaOHMolar mass of HCl = 36.4580.62 ×36.458/36 = 0.63ml0.63/36.458 = 0.0172mol/0.63 = 0.027mol/L= 0.63 × 0.027/35.3 = 0.0004820.62...
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Calculate the pH of the solution that results when mixing 20.0ml of 0.1750M HCl with 25.0ml of a_distilled water b_0.132M NaOH c_0.132M NH3 d_0.232M NaOH
a) pH = -lg [H + ] C M = n/V n (HCl) = 0.1750 · 20.0 = 3.5 mmol C M (HCl) = 3.5 / 45.0 = 0.08 M...
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If it takes 24.1 mL of a 0.638 M sodium hydroxide solution to neutralize 29.6 mL of a HCl solution, calculate the concentration of the HCl solution.
The balanced equation: NaOH + HCl → NaCl + H2O So, the ratio of reagents is 1:1. Amount of NaOH: 0.638 ∙ 24.1 = 15.3758 mmol Amount of HCl is...
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if it takes 80.0ml of 1.500 M KOH to neutralize120.0ml of given H3PO4 solution, what is the molarity of this phosphoric acid solution?
The molarity is 0.33 M.The equation is:3KOH + H3PO4 → K3PO4 + 3H2OThe number of moles of KOH = 1.5mol/L*0.08L = 0.12 molFrom the equation the number of moles of...
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Calculate the pH in the titration of 10.00mL of 1.0M HCl with 1.0M NaOH after the addition of 0.0mL NaOH?
You're titrating hydrochloric acid, HCl, a strong acid, with sodium hydroxide, NaOH, a strong base, so right from the start you should know that the pH at equivalence point must...
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34.62 mL of a 0.3 M Mg(OH)2 solution are needed to neutralize a 15-mL solution of HCl on unknown concentration. Calculate the concentration of HCl solution.
Mg(OH)2+2HCl=MgCl2+2H2O1.Trace by finding the amount of Mg(OH)2. To do this, we multiply the molarity by the volume (liters): 0.03462litres *0.3 mol/litres= 0.010386 mol Mg(OH)22.based on the reaction we find the amount...
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If takes 54 ml of 0.1 M NaOH to neutralize 125ml of an HCl solution what is the concentration of HCl
Using M1V1 = M2V2M2 = (M1V1)/V2M2 = (0.1×54)/125 MWhich is equal to 0.0432M
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What mass of NaOH(s) must be added to 300 mL of HCl 0.25 M in order to completely neutralize this acid? 2 HCl + NaOH → NaCl + H<sub>2</sub>O
Solution:The balanced chemical equation:HCl + NaOH → NaCl + H2OAccording to the equation above: n(HCl) = n(NaOH)Molarity of HCl = Moles of HCl / Solution volumeHence,Moles of HCl = n(HCl) = Molarity...
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